Acetic acid partially dissociates according to the reaction below. HC₂H3O2 + H₂O(1) H3O+ + C₂H30₂ ⇒ K = 1.8 x 10-5 @ 25°C Calculate the equilibrium concentrations of the components based on a 0.21 M acetic acid solution. What is the concentration of H3O+? [H3O+] = [?] x 10⁰ M Exponent (yellow) Coefficient (green) Enter
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- It is found that 8.70e-09 g of Ga(OH)3 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Ga(OH)3.The Ksp of Y2(CO3)3 at 25 oC is 1.03e-31. What is the molar solubility of Y2(CO3)3?The acid-dissociation constant for benzoic acid (C6H5COOH)is 6.3 x 10-5. Calculate the equilibrium concentrations ofH3O+, C6H5COOH-, and C6H5COOH in the solution if the initialconcentration of C6H5COOH is 0.050 M.1.For the aqueous reaction A + B à C + D, the equilibrium concentrations in moles per liter are [A] = 0.002, [B] = 0.005, [C] = 0.00004 [D] = 0.00025 i. What is the equilibrium constant Keq? ii. What is the dissociation constant pK? a. The partial pressure of gas A is 10 ppmv. It has a Henry’s constant for dissolution in water of KH = 0.02
- 1. Given the following equilibria and equilibrium constants. Ca2+ + 2C2O42- + H2O <-> CaC2O4•H2O(s) Ksp = 1.96×10-8 H2C2O4 <-> H+ + HC2O4- Ka1 = 5.60×10-2 HC2O4- <-> H+ + C2O42- Ka2 = 5.42×10-5 Which species would increase upon the addition of 0.1 M HCl(aq)? 2. Solid Mn(OH)2(s) is added to 1.0 liter of distilled water. What is the concentration of Mn2+ in the solution? The Ksp for Mn(OH)2(s) is 1.6×10-13. 3. Solid Mn(OH)2(s) is added to 1.0 liter of a 0.01 M NaOH solution. What is the concentration of Mn2+ in the solution? The Ksp for Mn(OH)2(s) is 1.6×10-13. 4. Most sulfide compounds of transition metals are very insoluble. However, the solubility products vary over a wide range and separations of metal sulfides can be accomplished by using the pH of the solution to control the S2- concentration.…(a) If the molar solubility of Tl2S at 25 oC is 5.31e-08 mol/L, what is the Ksp at this temperature?Ksp = (b) It is found that 1.75e-06 g of Cu3(AsO4)2 dissolves per 100 mL of aqueous solution at 25 oC. Calculate the solubility-product constant for Cu3(AsO4)2.Ksp = (c) The Ksp of BaCO3 at 25 oC is 2.58e-09. What is the molar solubility of BaCO3? solubility = ____ mol/LThe equilibrium constant for the reaction2Fe3+(aq) + Hg22+(aq) ⇌ 2Fe2+(aq) + 2Hg2+(aq)is Kc = 9.1×10-6 at 25.0°C. What is ΔGo at this temperature?
- The solubility product for Pb(Cl)2 is K = 1.60 * 10-5, the solubility product forPb(F)2 is K = 3.70 * 10-8 , and K for the following reaction is 1.98 * 10-4:Pb(Cl)2 (s) + 2 HF ⇌ PbF2 (s) + 2 H+ + 2Cl-Calculate the dissociation constant for H1) Write the pertinent reactions associated with the question2) Write the equilibrium constantexpression for each chemicalreaction.3) Write the mass balance equations4) Write the charge balance equation5) Count the equations andunknowns.6) SolveYou are on a new planet and discover a substance, Z2O that undergoes autoionization just like water on Earth. Z2O + Z2O ⇌ Z3O+ + OZ– Through a series of experiments, you determine the equilibrium constant (Kx) for this autoionization reaction at various temperatures. The value of Keq at 26.8ºC is 6.9 x 10-14. What is the pZ of the pure substance at this temperature? (pZ = -log(Z3O+) Report your answer to the hundreths placeThe acid-dissociation constant for chlorous acid (HClO2) is1.1 x 10-2. Calculate the concentrations of H3O+, ClO2-,and HClO2 at equilibrium if the initial concentration ofHClO2 is 0.0125 M.
- Give only typing answer with explanation and conclusion to all parts A. When 18.0 mL of a 6.77×10-4 M ammonium sulfate solution is combined with 18.0 mL of a 3.79×10-4 M silver nitrate solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to____ B.When 25.0 mL of a 2.00×10-4 M calcium bromide solution is combined with 18.0 mL of a 4.07×10-4 M ammonium phosphate solution does a precipitate form? (yes or no) For these conditions the Reaction Quotient, Q, is equal to ____Given below is the dissociation of NH3 in water having a Kb value of 1.8 × 10-5. The reaction started with the equilibration of 0.65 M NH3. A common ion that is 0.25 M NH4Cl, was added to the initial solution and waited for some time for the reaction to reach equilibrium once again. NH3(aq) + H2O(l) ↔ NH4+(aq) + OH-(aq) Determine the pH of the solution given after the addition of the common ion. The Kw of water is 1.0 × 10-14.Using the appropriate Ksp values, find the concentration of NO3− ions in the solution at equilibrium after 700 mL of 0.40 M aqueous Cu(NO3)2 solution has been mixed with 500 mL of 0.30 M aqueous KOH solution. (Enter in M.) (Ksp for Cu(OH)2 is 2.6x10-19).